• Gas laws come from 150 years of experimental work by different scientists. These are empirical results.
• We're gonna dive into a theoretical model, the kinetic model, and compare it to those empirical results.

Based on a series of assumptions.

• Gas Particles: Gases are just a big collection of identical particles (atoms or molecules).
  • 🎈 Real-world example: Think of it as a room full of bouncing balls, all looking and weighing the same.
• Constant Random Motion: These particles are always moving and their paths are random.
  • 🎈 Real-world example: Imagine kids running aimlessly in a playground.
• Negligible Particle Volume: The total space taken up by the particles is tiny compared to the entire space the gas occupies.
• Bouncy Collisions: Particles bounce off each other and container walls without losing energy (elastic collisions).
  • 🎈 Real-world example: Imagine rubber balls bouncing around a room without getting deflated.
• No Intermolecular Force: No energy-draining attractions or repulsions between particles, except when they crash.
• Super Fast Collisions: When particles collide, they do it super fast. So fast, you can't even notice.
• No External Forces: Forces like gravity don't matter in this model.

• If a particle hits a wall straight on, it bounces back with the same speed but in the opposite direction.
• The particle's momentum change is double its original (because it reversed).
  • 🎈 Real-world example: Imagine throwing a ball at a wall. It comes back to you with almost the same speed it was thrown, but in the opposite direction.
• In a gas, many such particles hit and rebound from walls, exerting a force.

1. If one particle exerts a force of \(\frac {mv^2_x}{L}\)​​ on the wall, imagine how much force N number of such particles would exert! That's\(\frac {mv^2_x}{L}\)​​ for all of them.
2. v² = v^2_x ​+ v_y² ​+ v_z²​ is the speed equation from the three speed components.